The melting point of a solid depends on the strength of the intermolecular forces holding the particles in place. In molecular solids, the intermolecular forces are typically weaker than the ionic forces in ionic solids. This is because molecular solids are held together by van der Waals forces, dipole-dipole forces, or hydrogen bonding, whereas ionic solids are held together by strong electrostatic forces between positively and negatively charged ions.

The strength of the intermolecular forces in molecular solids also depends on the size and shape of the molecules. Smaller molecules with simpler shapes tend to have weaker intermolecular forces than larger molecules with more complex shapes. This is because larger molecules with more complex shapes have more surface area for contact between molecules, which allows for more intermolecular interactions.

As a result of the weaker intermolecular forces, molecular solids typically have lower melting points than ionic solids. The melting point of a molecular solid is typically below 100°C, whereas the melting point of an ionic solid is typically above 100°C.

Here are some examples of molecular solids with low melting points:

* Iodine (I2): Melting point = 113.7°C

* Naphthalene (C10H8): Melting point = 80.2°C

* Benzene (C6H6): Melting point = 5.5°C

Here are some examples of ionic solids with high melting points:

* Sodium chloride (NaCl): Melting point = 801°C

* Potassium chloride (KCl): Melting point = 770°C

* Calcium fluoride (CaF2): Melting point = 1402°C